CHEM102 Lecture Notes - Lecture 24: Reaction Calorimeter, Dave Coverly, Exothermic Reaction

• School: University of Alberta
• Department: Chemistry
• Course: CHEM102
• Professor: Yoram Apelblat

Document Summary

= q p v restricting work to be only the work of a gas. but. Measure heat at constant volume get u. Ch4 (g) + 2 o2 (g) co2 (g) + 2 h2o (g) + heat. N2 (g) + o2 (g) + heat 2 no (g) rxn that absorbs heat. Define enthalpy, h, as h = u + pv. Since we can"t really measure absolute energies, then the equation to use is. U, p, v are state functions h is a state function. For a process under constant pressure and the work is only pv work. H = (u + pv) = u + (pv) = q + w + (pv) = Qp where: qp = heat at constant p. Measure heat at constant pressure get h. Go back to the earlier figure and add. Heat can only be exchanged between the reaction and the calorimeter, but not with the surroundings. qreaction + qcalorimeter = 0.